In Class 11 Chemical Bonding, Hybridization is a crucial concept introduced by Linus Pauling to explain the shape and geometry of molecules (like why Methane, CH₄, is a perfect tetrahedron).
Concept: Mixing pure atomic orbitals to form new hybrid orbitals.
Result: The new hybrid orbitals have identical energy and shapes.
Purpose: It explains the stable molecular geometry and bond angles of chemical compounds.
Main types: sp (linear), sp² (trigonal planar), sp³ (tetrahedral).
Hybridization is defined as the process of mixing two or more atomic orbitals belonging to the same atom, which have slightly different energies, to produce an entirely new set of orbitals of equivalent energy and identical shape. These new orbitals are called Hybrid Orbitals.
Imagine you have one bucket of red paint (an 's' orbital) and three buckets of white paint (three 'p' orbitals). If you mix them all together, you don't have red and white anymore; you get four identical buckets of light pink paint (four 'sp³' hybrid orbitals).
The type of hybridization depends on which orbitals are mixed:
Hybridization is the phenomenon of mixing atomic orbitals of slightly different energies of the same atom to form a new set of identical orbitals with equivalent energy and shape, called hybrid orbitals.
Hybridization occurs to minimize the repulsion between electrons and to form stronger, more stable covalent bonds, giving the molecule a specific geometric shape.
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